1. Warm-Up What is a solution? Very small particles Evenly distributed
Do not separate

2. Solutions

3. Solution Process

4. Solution Vocabulary Solvent – liquid that is doing the dissolving
Solute – substance that dissolves in the liquid solvent
Gas, liquid, or solid
Rate of dissolution will speed up by same factors that increase the rate of reaction:
Higher temperature
Increased surface area of solute
Increased concentration of solute

5. Saturation Saturated solutions contain as much solute as possible
Unsaturated solutions can dissolve more solute
Supersaturated solutions have dissolved more solute than is normally possible
Formed by cooling down a saturated solution

6. Saturation Line represents a saturated solution at a given temperature
Above the line is supersaturated
Below the line is unsaturated
Temperature Effect:
Solids dissolve better at high temperatures
Gases dissolve better at low temperatures
Also at high pressures

7. Colligative Properties
When a solid dissolves in a liquid, it stabilizes the liquid phase! This effects 4 physical properties of the liquid:
Boiling Point Elevation
Freezing Point Depression
Vapor Pressure Lowering
Osmotic Pressure Increasing

8. Colligative Properties
Boiling Point Elevation
Freezing Point Depression
The boiling point of a liquid increases as it dissolves solid particles.
The freezing point of a liquid decreases as it dissolves solid particles.

9. Vapor Pressure Lowering
Vapor pressure is the pressure exerted by a vapor in equilibrium with its liquid form
A liquid boils when its vapor pressure is equal to the atmospheric pressure
The vapor pressure of a liquid decreases as it dissolves solid particles.

10. Osmotic Pressure Increasing
Osmotic pressure is the amount of pressure that needs to be applied to a solution to prevent water from flowing in through a semi-permeable membrane.
The osmotic pressure of a liquid increases as it dissolves solid particles.

11. Warm-Up ABBREVIATE PROMPTS!!
Which substances are gases at room temperature?
If 100 g of sodium nitrate is completely dissolved in 100 g of water at 20oC, what type of solution is formed?
If 80 g of hydrogen chloride are dissolved in 200 g of water at 70oC, what type of solution is formed?

12. Warm-Up
Define “Molarity” in your own words.

13. Molarity 𝐌𝐨𝐥𝐚𝐫𝐢𝐭𝐲 𝐌 = 𝐀𝐦𝐨𝐮𝐧𝐭 𝐨𝐟 𝐒𝐨𝐥𝐮𝐭𝐞 (𝐦𝐨𝐥) 𝐕𝐨𝐥𝐮𝐦𝐞 𝐨𝐟 𝐒𝐨𝐥𝐮𝐭𝐢𝐨𝐧 (𝐋)
A dilute solution has a little solute, LOW molarity
A concentrated solution has a lot of solute, HIGH molarity
𝐌𝐨𝐥𝐚𝐫𝐢𝐭𝐲 𝐌 = 𝐀𝐦𝐨𝐮𝐧𝐭 𝐨𝐟 𝐒𝐨𝐥𝐮𝐭𝐞 (𝐦𝐨𝐥) 𝐕𝐨𝐥𝐮𝐦𝐞 𝐨𝐟 𝐒𝐨𝐥𝐮𝐭𝐢𝐨𝐧 (𝐋)

14. Practice!
What is the molarity of a solution formed by mixing 10.0 g H2SO4 with enough water to make mL of solution?

15. Practice!
Vinegar is a solution of acetic acid. What mass of acetic acid must be used to prepare L of vinegar (1.39 M)?

16. Dilutions
You may use the equation below to determine how you should dilute a solution of known concentration:
M 1 V 1 = M 2 V 2
Note: Volume
units must
match!

17. Practice!
How do you make mL of 3.0 M sulfuric acid solution using an 18.0 M stock solution of sulfuric acid?

18. Practice!
Ms. Hall dilutes 25.0 mL of 12.0 M hydrochloric acid to mL. What is the concentration of the dilute solution?

19. Making Solutions
Add enough water to a volumetric flask to almost fill the bottom of the flask.
Add the calculated amount of solute to the flask and swirl to dissolve in the water.
Fill the flask with water to the etched line on the neck and mix well.

20. Diluting Solutions
Add the calculated amount of concentrated solution to a volumetric flask.
Fill the flask with water to almost fill the bottom of the flask and mix well.
Fill the flask with water to the etched line on the neck and mix well.

21. Diluting Solutions
Practice! 1) Write a detailed procedure that describes how you would create one of the solutions on the front of the notes.